14797-55-8

Usage

Chemical Description

Nitrate and nitrite are secondary products that can be produced during the decomposition of liquid nitric peroxide by alkalis and acids.

Uses

Used in Meat Curing Industry:
Nitrate is used as a curing agent for developing and stabilizing the pink color associated with cured meat. It also has an effect on flavor and functions as an antioxidant.
Used in Pharmaceutical Industry:
Nitrate is used in the treatment of angina pectoris and in the manufacture of inorganic and organic nitrates and nitro compounds for various applications.
Used in Fertilizer Industry:
Nitrate is used in fertilizers, contributing to plant growth and development.
Used in Chemical Industry:
Nitrate is used in the manufacture of nitrites, nitrous oxide, explosives, pyrotechnics, matches, freezing mixtures, and special cements.
Used in Food Industry:
Nitrate serves as a coloring agent and preserving additive in the food industry.
Used in Industrial Applications:
Nitrate is used for coagulation of latexes, in the nuclear industry, and for odor (sulfide) and corrosion control in aqueous systems.
Chemical Properties:
Nitrate is a colorless liquid at room temperature and is involved in the nitrogen cycle in the environment and the body. It plays a significant role in inducing toxicity after its formation from nitrate, which is a subject of public health interest. The World Health Organization (WHO) guideline of 50 ppm and the US maximum contaminant level (MCL) of 45 ppm for nitrate in drinking water have been established to protect infants from methemoglobinemia, also known as blue baby syndrome.

Air & Water Reactions

Most are water soluble.

Reactivity Profile

Mixtures of metal/nonmetal nitrates with alkyl esters may explode, owing to the formation of alkyl nitrates; mixtures a nitrate with phosphorus, tin (II) chloride, or other reducing agents may react explosively [Bretherick 1979. p. 108-109].

Hazard

Moderately toxic.

Health Hazard

Inhalation, ingestion or contact (skin, eyes) with vapors or substance may cause severe injury, burns or death. Fire may produce irritating, corrosive and/or toxic gases. Runoff from fire control or dilution water may cause pollution.

Fire Hazard

These substances will accelerate burning when involved in a fire. Some may decompose explosively when heated or involved in a fire. May explode from heat or contamination. Some will react explosively with hydrocarbons (fuels). May ignite combustibles (wood, paper, oil, clothing, etc.). Containers may explode when heated. Runoff may create fire or explosion hazard.

Environmental Fate

Nitrate (NO3 -), a product of nitrogen oxidation, is a naturally occurring ion in the environment and integrated into complex organic molecules such as proteins and enzymes required by living systems. Nitrate is a more stable form of oxidized nitrogen than nitrite; however, it can be reduced by microbial action to nitrite, which, in turn, can be reduced to various compounds or oxidized to nitrate by chemical and biological processes. Nitrates occur naturally in soil from microbial oxidation of ammonia derived from organic nitrogenous materials such as plant proteins, animals, and animal excreta. Other source contributions are wastewater, septic tank runoffs, airborne nitrogen compounds emitted by industry and automobiles, nitrogen fertilizer, and manure from animal feeding. Nitrate in groundwater is generally found below 10 ppm, with higher levels in areas of high agricultural activities.

Toxicity evaluation

The acute oral LD50 values for sodium nitrate range from 2480 to 9000 mg kg-1 in rats, mice, and rabbits. Acute, subchronic, and chronic animal toxicity studies showed low toxicity for nitrate as sodium or potassium nitrate. A long-term study showed a slight depression in growth rate. Nitrite, but not nitrate, is capable of inducing methemoglobinemia (see Nitrites, for more details). Nitrate has been reported to be associated with thyroid effects in experimental animals and humans. Possible mode of action includes inhibition of iodine uptake to thyroid, serum T3 and T4 changes, and tissue T3 changes. However, there is a lack of knowledge on the differences in the mode of action to permit animal-to-human extrapolation. While the data indicate humans and rats exhibit similar dose–response relationships in acute inhibition of thyroidal iodide uptake, they show differences in thyroid hormone response following iodide uptake inhibition. Comparative data are needed for serum and brain tissue levels of thyroid hormones and characterization of the dose–response relationship between changes of thyroid hormone levels and adverse effects. Early experimental and field studies in mammals have found inorganic nitrate to be goitrogenic. The effects were observed in rats following oral and parenteral administration of potassium and sodium nitrate, whereas antithyroid effects were also reported in sheep and pigs administered potassium nitrate. Nitrate exposure through diet or drinking water caused functional and histological changes to the thyroid gland in rats and pigs. More recent investigations between 2000 and 2010 reported changes in thyroid and thyroid activity following exposure to nitrate. In these more recent studies, nitrate exposure has consistently resulted in increases in thyroid weight and/or changes to the follicle cell; however, the reported thyroidal hormone changes have not been as consistent. The studies reported increased thyroid weights with a decrease in thyroid hormones (i.e., T3 and T4) and/or decrease in thyroid stimulating hormone. However, not all the results are consistent with the expected outcome of a sodium–iodide symporter (NIS) inhibitor, which can be seen as supplementation of iodine in the diet that did not result in thyroid changes. Overall, the data support that nitrate impairs thyroid function involving the hypothalamic–pituitary–adrenal axis.

InChI:InChI=1/NO3/c2-1(3)4/q-1

Upstream product

• 645-48-7 1-phenyl-3-thiosemicarbazide 
• 7732-18-5 water 
• 10102-43-9 nitrogen(II) oxide 
• 10102-44-0 Nitrogen dioxide 
• 7727-37-9 nitrogen 
• 7664-93-9 sulfuric acid 
• 7697-37-2 nitric acid 
• 29817-79-6 nitrogen-15 
• 1173020-41-1 ⁽¹⁴⁾-nitrogen 
• 10024-97-2 dinitrogen monoxide 
• 12775-96-1 copper 
• 7632-00-0 sodium nitrite 
• 201230-82-2 carbon monoxide 
• 1333-74-0 hydrogen 

Downstream Products

• 14900-04-0 triiodide^(1-) 
• 16043-45-1 titanium(IV) 
• 7727-37-9 nitrogen 
• 13907-45-4 chromate(VI) ion 
• 63717-99-7 trans-Rh(PCy₃)2(CO)(nitrate) 
• 71882-16-1 trans-Rh(PPh₃)2(CO)(nitrate) 
• 22654-78-0 trans-Rh(PPh₃)2(CO)(nitrate) 
• 128872-17-3 {Co(CO)3(P(C₆H₅)3)2}⁽¹⁺⁾*NO₃^(1-)={Co(CO)3(P(C₆H₅)3)2}NO₃ 
• 13985-99-4 (C₅H₄N)2B(C₆H₅)2⁽¹⁺⁾*NO₃^(1-)={(C₅H₄N)2B(C₆H₅)2}NO₃ 
• 14058-12-9 (C₁₂H₈N₂)B(C₆H₅)2⁽¹⁺⁾*NO₃^(1-)={(C₁₂H₈N₂)B(C₆H₅)2}NO₃ 
• 1254205-41-8 C₃₀H₂₄N₆O₄S₂*NO₃^(1-) 
• 1268518-27-9 [2-(4-nitrophenyl)amino-1,3-diazaferrocenophane(+1H)]NO₃ 

Relevant academic research and scientific papers

Chemical and Electrochemical Oxidation of Solutions of Silver Nitrate in Acetonitrile

In anhydrous acetonitrile the unstable, brown species Ag(NO3)42-, I, can be produced either by the electrolysis of silver nitrate or by the equilibrium reaction N2O5 + Ag+ + 3NO3- ->/-3.The ESR spectrum of I at 77 K is that of a Ag(II) ion in a field with pronounced axial distortion.Its resonance Raman spectrum indicates square-planar coordination of the metal ion by unidentate nitrate ligands.The complex decomposes to form cyanomethyl nitrate and nitric acid by the rate law -d/dt = k/->.In the presence of p-xylene a major organic product is p-methylbenzyl nitrate.Equilibrium and electrochemical studies lead to estimated ΔG0298 values for the free radical and ionic dissociation pathways of N2O5 in acetonitrile solution of +38 and -26 kJ, respectively.

Kinetics and mechanism of oxidation of nitrous acid by chlorite ion

Although the oxidation of nitrite by chlorite both stoichiometrically and kinetically is a fairly simple reaction when nitrite is in excess and the pH is above 4, it becomes exceedingly complex in acidic solution containing chlorite in excess. Cl2O2 appears to be a key intermediate, the transitory formation of which explains both the formation of ClO2 and peculiar three-extrema E versus time curve. Assuming that the electrode process on the bright Pt electrode is HOCl + e- + H+ = Cl2 + H2O, the reaction is an oligooscillatory one in which the concentration of HOCl exhibits three extrema at most.

Nucleophile Assistance of Electron-Transfer Reactions between Nitrogen Dioxide and Chlorine Dioxide Concurrent with the Nitrogen Dioxide Disproportionation

The reaction of chlorine dioxide with excess NO2- to form ClO2- and NO3- in the presence of a large concentration of ClO2- is followed via stopped-flow spectroscopy. Concentrations are set to establish a preequilibrium among ClO2, NO2-, ClO2-, and an intermediate, NO2. Studies are conducted at pH 12.0 to avoid complications due to the ClO2-/NO2- reaction. These conditions enable the kinetic study of the ClO2 reaction with nitrogen dioxide as well as the NO2 disproportionation reaction. The rate of the NO2/ClO2 electron-transfer reaction is accelerated by different nucleophiles (NO2- > Br- > OH- > CO32- > PO43- > ClO2- > H 2O). The third-order rate constants for the nucleophile-assisted reactions between NO2 and ClO2 (kNu, M -2 s-1) at 25.0 °C vary from 4.4 × 10 6 for NO2- to 2.0 × 103 when H2O is the nucleophile. The nucleophile is found to associate with NO2 and not with ClO2 in the rate-determining step to give NuNO2+ + ClO2-. The concurrent NO2 disproportionation reaction exhibits no nucleophilic effect and has a rate constant of 4.8 × 107 M-1 s -1. The ClO2/NO2/nucleophile reaction is another example of a system that exhibits general nucleophilic acceleration of electron transfer. This system also represents an alternative way to study the rate of NO2 disproportionation.

Spontaneous reactions and reduction by iodide of peroxynitrite and peroxynitrate: mechanistic insight from activation parameters

Thermal and pressure activation parameters are reported for the decomposition of peroxynitrate, isomerization of peroxynitrite, and their reduction by iodide in aqueous solutions. The spontaneous decomposition reactions are characterized by activation ent

HYPOCHLORITE OXIDATION OF AMMONIA. EFFECTIVE REMOVAL OF AMMONIA FROM WASTE WATER BY UV-IRRADIATION.

The hypochlorite oxidation of ammonia giving rise to nitrogen evolution was carried out in the dark or under irradiation in order to study the reaction mechanism and application to waste water treatment. UV-irradiation accelerates remarkably the rate of decomposition of unfavorable chloramines. The acceleration covers the pH region 2-12, where corresponding dark reactions are slow. The irradiation also affects the formation of byproducts such as NO//2** minus and NO//3** minus , the effect being a slight increase in NO//2** minus formation in the pH range 2-12. These results suggest an effective industrial application to avoid eutrophication in seas and lakes. The irradiation effect is discussed in relation to reaction mechanism, in which the irradiation possibly facilitates the N-N bond formation after chloramine formation.

Enhanced photocatalytic degradation of methylene blue under vacuum ultraviolet irradiation

A vacuum ultraviolet (VUV) lamp was used as the irradiation of photocatalysis to enhance the degradation of methylene blue (MB), a model dye compound. In contrast to photocatalysis under 254 nm UV irradiation (UV/TiO 2), photocatalysis under VUV irradiation (VUV/TiO2) exhibited much higher efficiency in MB degradation and mineralization and needed less TiO2 dosage. The rate constant of MB degradation in VUV/TiO2 (0.0793 min-1) is about 4 times of that of UV/TiO2 (0.0205 min-1). The MB mineralization rate is also greatly increased from 12.5% in UV/TiO2 to 47.7% in VUV/TiO 2 after 60 min of irradiation. Multiple advanced oxidation processes including photocatalytic oxidation and VUV photo-oxidation coexist in VUV/TiO2 to substantially produce highly reactive species (such as OH and energetic photons), which is responsible for efficient degradation and mineralization of MB.

NMR study of reactions between Pd, Ru, and Rh nitrite complexes with sulfamic acid

Reactions of nitrite complexes of Pd, Ru, and Rh with sulfamic acid were studied by the 14, 15N, and 17O NMR method. Chemical shifts were assigned, and the predominant forms of the complexes were established. The reaction products at room temperature are cis-nitroaqua complexes. Coordination of the sulfamate ion upon storage for a long time or on heating was detected.

The role of cobalt oxide or magnesium oxide in ozonation of ammonia nitrogen in water

In this study, the reaction mechanisms for ozonation of ammonia nitrogen in the presence of Co3O4 or MgO were investigated. For the reaction over Co3O4, Cl– in the reaction solution was indispensable and ClO– was formed by a non-catalytic oxidation of Cl–. Co3O4 promoted the reaction of NH4+ with ClO– to give the products including NO3–, chloramines and gaseous products. In contrast, Cl– was unnecessary for the reaction with MgO. pH of the reaction solution was maintained at around 9 throughout the reaction owing to partial dissolution of MgO. Ammonia nitrogen was decomposed to mainly NO3– by non-catalytic radical reaction involving OH·, which was formed by the reaction of OH– with O3 in weakly basic solution. To keep the reaction solution weakly basic, H+ formed with the decomposition of NH4+ was neutralized. As a result, about the same amount of Mg2+ as that of decomposed ammonia nitrogen was dissolved.

Nanopore enriched hollow carbon nitride nanospheres with extremely high visible-light photocatalytic activity in the degradation of aqueous contaminants of emerging concern

Construction of highly efficient hollow nanosphere photocatalytic systems has been strongly attracting the attention of researchers. In the present work, nanopore enriched hollow carbon nitride nanospheres (HCNNSs) with a smaller particle size (200 nm) and a thinner shell thickness (40 nm) are successfully fabricated by a silica-nanocasting strategy. Such unique structures possess many advantages such as large BET surface area (122 m2 g-1), high light-harvesting ability, fast charge separation and transfer efficiency, plentiful exposed active sites and enhanced oxidation ability of photogenerated holes (h+VB). Therefore, HCNNSs in smaller sizes (HCNNS-200) exhibit extremely excellent visible-light photocatalytic efficiency towards the degradation of contaminants of emerging concern, e.g. levofloxacin (LEVO), in comparison with bulk g-C3N4 and HCNNSs in larger sizes (HCNNS-500). And it takes less than 10 min to finish the degradation of LEVO. The experimental results including those from indirect chemical probing, electron spin resonance, ion chromatography and high performance liquid chromatography-mass spectrometry confirm that h+VB and O2- are the active species that are responsible for the mineralization of LEVO to NO3-, F-, H2O and CO2 under visible-light irradiation. Additionally, the degradation pathway of LEVO in the HCNNS-200 photocatalytic system is also proposed. It is expected that HCNNS-200 can be used as a promising photocatalyst for environmental remediation.

Cold atmospheric plasma activated water as a prospective disinfectant: The crucial role of peroxynitrite

The socio-economic, environmental, and health implications of diseases caused by pathogenic microorganisms and their treatment using conventional antimicrobials are significant. The increasing resistance to antibiotics and detrimental biological side effects of many common antibiotics on human health and on the ecosystem have driven the search for new cost-effective and highly-efficient sterilization treatments and agents that are more environmentally benign. Plasma activated water (PAW), a product of cold atmospheric plasma reacting with water, is a promising broad-spectrum biocidal agent whose biochemical activity is attributed to the presence of a rich diversity of highly reactive oxygen and nitrogen species (RONS). The transient activity of PAW, where PAW reverts to water within days of storage and application, suggests that it can become a green alternative to conventional chemical treatment methods, yet the issues of scale up and the not fully understood mechanism of activity remain. In this study, we sought to explore the antibiotic potential of PAW generated from a plasma jet in a continuous flow reactor and determine the individual and combined contribution of thus-generated reactive chemistries in PAW for organism inactivation. Treatment of Escherichia coli with PAW led to more than a 4-log reduction, while exposure to an equivalent single dose of hydrogen peroxide (H2O2), nitrate (NO3-) or nitrite (NO2-) to that found in PAW failed to attain the same level of reduction. Peroxynitrite was identified as a critical bioactive species, particularly under acidic conditions, originating from the synergistic plasma effects (like the reactions of H2O2, NO3-, NO2- and other existing short-lived species like OH radicals in PAW). This research successfully demonstrated the possibility of PAW being an effective environmentally benign disinfectant, the activity of which is closely linked to the generation of peroxynitrite, providing much needed insights into the fundamental aspects of PAW chemistry required for optimisation of the biochemical activity of PAW and translation of this decontamination strategy into real life applications.